1.) average number of moles of NaOH dispensed 3,) Based on your coarse titration
ID: 998345 • Letter: 1
Question
1.) average number of moles of NaOH dispensed
3,) Based on your coarse titration volume, do you expect the acetic acid solution to have a higher or lower concentration than the NaOH solution?
please help with these 2 questions
Part 1: Prepare the NaOH Solution
Lab Results
How many mL of water were used to prepare the NaOH solution?
Data Analysis
Calculate the molarity of the NaOH solution. The molar mass of NaOH is 39.997 g/mol.
Calculate the amount of benzoic acid to be neutralized by 20.00 mL NaOH solution, in both moles and grams. The molar mass of benzoic acid is 122.12 g/mol.
Part 2: Perform a Coarse Titration
Lab Results
Record the following data from your course titration in the table below.
Data Analysis
How do you expect your coarse titration volume to compare to your fine titration volumes?
Part 3: Perform Fine Titrations
Lab Results
Record the volume of NaOH solution dispensed in the 3 fine titrations.
Data Analysis
Calculate the average concentration of the NaOH solution, using the average volume of NaOH solution dispensed in the 3 fine titrations. Report your answer using enough significant figures to distinguish it from the expected concentration of 0.100 M.
V = (V1 + V2 + V3) / 3
V = (20.03 mL + 20.06 mL + 20.02 mL) / 3 = 20.04 mL
M = n / V = 0.00200 moles / 0.02004 L = 0.0998 M
Learning objective: Determine the concentration of a solution.
20.21= ----> 0.0999M
Experiment 2: Use the Standardized NaOH Solution to Determine the Concentration of an Acid
Part 1: Perform a Coarse Titration
Lab Results
What was the pH at the end point of the coarse titration?
Data Analysis
Based on your coarse titration volume, do you expect the acetic acid solution to have a higher or lower concentration than the NaOH solution?
Part 2: Perform Fine Titrations
Lab Results
For the 3 fine titrations of the acid of unknown concentration, fill in the following data.
Data Analysis
Calculate the following quantities and record the data in the table below.
Conclusions
Phenolphthalein is pink over the range of pH 8 – 12. Why was it a useful indicator of when the equivalence point was reached?
Suppose a student titrated a sample of monoprotic acid of unknown concentration using a previously standardized solution of NaOH.
Given the data in the figure above, what is the concentration of the unknown acid?
0.0617M
Lab NOTES:
ex1
Take sodium hydroxide from the Materials shelf and add 0.800 g to the beaker.
Take water from the Materials shelf and add 200 mL to the beaker.
Ph 2.96
inital volume in burett
inital volume 50ml
1.) volume43.78mL
volumes dispenced =6.22ml
2. volume =38.05
volume dispenced =11.95ml
3.)volume = 32.06
volume dispenced=17.94
4.28.89ml
volume dispenced=21.11ml
ph=10.95
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Ex 2
inital ph= 2.96
volume30.33
dispence 20.05
1. volume 39.92ml
volume dispenced=10.08
2.volume 29.66
voiume dispence 20.34
final ph10.43
initial valume in burett 50ml
--------------------
ex3
final ph9.43
volume 30.28
volume dipenced=20.00
----------------------------------------------------------------------
2nd Ex
initial ph 3.11
volume 50
1. volume 48.95mL
dispenced 1.05mL
ph 3.87
2. volume 45.88
dispenced 4.12
ph 4.67
3 volume 42.99
dispenced 7.01
ph 5.29
4 volume 39.93
dispence 10.07
ph 11.45
--------------------
F1
final ph 9.99
volume 59.11
dispenced 9.05
F2
ph 9.59
volume 40.97
dispenced 9.03
f3
ph 9.50
volume 40.98
9.02
1.) average number of moles of NaOH dispensed
Explanation / Answer
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